True/ False: If “False”, explain why in complete sentences.

Select 2 oxygen atoms. a )How many valence electrons are in each oxygen atom? b)Is an oxygen atom a metal or a non-metal? C)Did the combination of these atoms create a covalent or ionic bond 'd)How are the valence electrons organized to form a bond between the atoms?e. How is this bond different from the bond in the fluorine molecule in question 1?

Draw a Lewis structure for SiF5- and answer the following questions based on your drawing. 1. For the central silicon atom: ... The number of lone pairs = ____   The number of single bonds = ____   The number of double bonds = ____   2. The central silicon atom (A,B, or C)   ... A. Obeys the octet rule   B. Has an incomplete octet.   C. Has an expanded octet.

Part II Practicing Coordinate Covalent Bonding for Molecular compounds. Example: Given the molecular compound SO, draw the molecular compound using the coordinate covalent bonding model. A. Calculate the total number of electrons. S = 1x 6 = 6 electrons O = 4 x 6 = 24 electrons Charge -2 = 2 electrons Total = 32 electrons B. Determine Center Atom (look for the single element) in this case S. C. Now make a single bond to all other elements to the central atom. You have used 8 electrons of the 32. 0- D. Place electrons around the atoms that are bonded to the central atom so that each will have 8 electrons around them (in this case each oxygen needs 6 more electrons or 3 pairs of electrons). : E. Make sure that the central atom has a full octet (8 electrons). In this case it does, so you are done. If not, one of the lone pairs of electrons from an outer atom will share a second pair of electrons with the center atom. Finally be sure that you have used all your electrons and NO MORE!